Exothermic

In thermodynamics, the word exothermic "outside heating" describes a process or reaction that releases energy usually in the form of heat, but it can also release energy in form of light (e.g. explosions), sound, or electricity (e.g. a battery). Its etymology stems from the Greek prefix ex-, meaning “outside” and the Greek word thermein, meaning “to heat”. The term “exothermic” was coined by Marcellin Berthelot. The opposite of an exothermic process is an endothermic process, one that absorbs energy in the form of heat.

The concept is frequently applied in physical sciences to chemical reactions, where chemical bond energy is converted to thermal energy (heat).

Overview

Exothermic refers to a transformation in which a system releases energy (heat) to the surroundings:

Q < 0

When the transformation occurs at constant pressure:

∆H < 0

and constant volume:

∆U < 0

In an adiabatic system (e.g. a system that does not give off heat to the surroundings), an exothermic process results in an increase in temperature.Perrot, Pierre (1998). A to Z of Thermodynamics. Oxford University Press. ISBN 0-19-856552-6. 

Exothermic processes

Some examples of exothermic processes are:Exothermic - Endothermic examples

• Condensation of rain from water vapor
• Combustion (for instance of a candle)
• Mixing water and strong acids
• Nuclear fusion

Implications for chemical reactions

Main article: exothermic reaction

Chemical exothermic reactions are generally more spontaneous than their counterparts, endothermic reactions. In a thermochemical reaction that is exothermic, the heat may be listed among the products of the reaction.

See also

Look up exothermic in
Wiktionary, the free dictionary.

• Endergonic
• Endergonic reaction
• Exergonic
• Exergonic reaction

External links

• http://chemistry.about.com/b/a/184556.htm Observe exothermic reactions in a simple experiment

References

This article is licensed under the GNU Free Documentation License. It uses material from Wikipedia